Manufacturing of Ti-6%Al and Ti-6%Al-4%V Alloys and Their Corrosion in Sodium Chloride Solutions

Abstract

The current research aims at the manufacturing of Ti-6%Al alloy and Ti-6%Al-4%V alloy using the mechanical alloying method and studying their corrosion behavior after various periods of immersions in 3.5% NaCl solutions. The fabricated alloys were also evaluated using spectroscopic techniques such as X-ray diffraction, scanning electron microscopy, and energy dispersive X-ray spectroscopy analyses. The corrosion behavior was studied using potentiodynamic polarization, electrochemical impedance spectroscopy, and chronoamperometric current-time electrochemical methods. It is confirmed that the presence of 4% V greatly decreases the uniform corrosion of the Ti-6%Al alloy as a result of the role of V in decreasing the cathodic, anodic, and corrosion current, and the rate of corrosion along with increasing the corrosion resistance. Increasing the time of immersion to 24 h and further to 48 h highly decreased the corrosion of the alloys. The presence of 4% V and extending the time of exposure thus increase the resistance against corrosion via decreasing the corrosion of Ti-6%Al alloy in the chloride test solution.

1. Introduction

Ti-base alloys have exceptional properties such as excellent mechanical properties, great biocompatibility, and outstanding corrosion resistance against various aggressive electrolytes [1,2,3,4,5]. For that, these alloys have been employed as a standard engineering materials in numerous industrial applications such as their potential use in medical, military, marine, and offshore application [4,5,6,7,8]. The fact that the good corrosion resistance to most corrosive media, the low density, and the high strength make various titanium alloys applicable to be employed in the marine industries and offshore structures [4,5,6,7,8]. The excellent corrosion resistance accounted for the Ti-base alloys has been claimed due to the surfaces of these materials having the ability to develop and form a continuous, highly adherent, stable, and protective titanium oxide layer (TiO₂). Under some anhydrous conditions, where there is no oxygen available, these like in sodium hydroxide solutions, sulfuric, and hydrochloric concentrated acid solutions, and, in some instants, the solutions containing chloride ions such as 3.5% NaCl solutions, the formed TiO₂ will damage and will not be able to be regenerated [7,9,10,11].

Numerous titanium base alloys have been reported to have a vital usage in the field of biomedical applications [12,13,14,15,16,17,18,19,20,21]. These alloys have been employed as screws for fracture fixation, artificial hip and knee joints, and bone plates to replace the failed tissues in the human bodies. An important issue in selecting the use of Ti alloys is the selection for the elements that can be alloyed with Ti, where these alloying elements have to be nontoxic metallic materials such as V, Nb, Ta, Zr, etc. [20]. Alloying Ti with these metals also enhances the resistance to corrosion and enhances the strength of α + β and the low-modulus β-type titanium alloy. One of these alloys, Ti6Al4V, has excellent resistance to corrosion and high mechanical and physical properties for which it has been chosen to be the most applicable Ti alloy in implantation systems [22,23,24,25]. This alloy was coated with titanium dioxide to be employed in the building of a new heart valve design [25]. Several Ti-base alloys like Ti6Al4V, Ti13Cu4.5Ni, and Ti6Al7Nb have been reported to be the ultimate choice for the use in orthopedic implants [26]. The reason for employing such alloys in the aforementioned uses is their corrosion resistance in vitro to form a stable oxide film in most aggressive environments [26,27,28,29,30,31,32]. The prevention of the release of Ti ions can be done via the formation of a uniform and a homogeneous coating layer of TiO₂ on the surface of Ti6Al4V alloy through its anodization in 1.0 M H₂SO₄ solution at 60 V [33,34,35,36].

This research study aims at the manufacturing of Ti-6%Al alloy and Ti-6%Al-4%V alloy from its raw powders by a high energy ball mall and a heat induction furnace using the mechanical alloying method. The electrochemical corrosion behavior of these alloys after 1 h, 24 h, and 48 h immersion in the corrosive solution using cyclic polarization (CPP), impedance spectroscopy (EIS), and chronoamperometric current-time (CCT) after stepping up the potential at fixed value techniques was carried out. The X-ray diffraction (XRD) patterns were collected to identify the composition and phase structure of the sintered alloys. SEM micrographs and EDX spectra were obtained after 48 h immersion in the test solution and then applying 300 mV (Ag/AgCl) for 30 min. It was expected that the presence of 4%V within the Ti-6%Al would increase its corrosion resistance via reducing its corrosion currents and corrosion rate after being immersed for various immersion times in the chloride medium.

2. Experimental Procedure

2.1. Supplies and Alloy Fabrication

A solution of 3.5% NaCl that was employed as the test solution was prepared from a sodium chloride salt that has 99.95% purity and was supplied by Sigma-Aldrich (Glasgow, UK). The alloys of Ti-6%Al and Ti-6%Al-4%V (percent of all alloying elements was in wt.%) were synthesized using 99.99% Ti, Al, and V powders, which were purchased for Sigma-Aldrich (Glasgow, UK). The required compositions of powders were mixed together in the presence of steel balls at a ratio 5 to 1 ball-to-powder. The mixture was placed in an evacuated jar of steel that accommodates for 80 mL. The jar was then placed in a desktop 220 V ball mill (Across International Co., Livingston, New Jersey NJ, USA). The operating conditions for the ball mill were 2000 rpm speed and 30 min milling time. After the ball milling, the powders were subject to sintering in a die made of graphite has 10 mm in diameter and 20 mm in length. The coupons were sintered using a high frequency induction heat sintering furnace (High-tech Zone, Zhengzhou City, Henan Province, China) under 40 MPa pressure of and 1200 °C temperature for 5 min.

2.2. Electrochemical Test Methods

The corrosion measurements were performed using an electrochemical cell with a three-electrode configuration; this cell accommodates for 250 mL NaCl solution. Both Ti alloys were used as the working electrodes. The employed reference and the counter electrodes were silver/silver chloride (Ag/AgCl) and a platinum sheet, respectively. The preparation of the working electrodes for the corrosion tests were reported in the previous work [37,38,39,40]. All electrochemical tests were obtained by the use of an Autolab workstation (PGSTAT302N, Metrohm, Amsterdam, Netherlands). The polarization tests were carried out in a potential range between −800 mV and 800 mV at scan rate of 1.66 mV/s [41,42]. The EIS experiments were obtained from the value of the open-circuit potential (E_OCP) and a frequency range started from 100,000 Hz to 0.01 Hz [38,39]. The potentiostatic (chronoamperometric, CCT) current-time data were gathered in NaCl solution after 48 h after immersion prior to applying a fixed potential value of 0.5 V for 0.5 h.

2.3. XRD Patterns, SEM, and EDX Analyses

Surface investigations were performed employing the XRD, SEM, and EDX techniques. The XRD spectra were performed by the use of D-8 Discover (Bruker, Berlin, Germany); the XRD spectra were carried out at 2°/min scan rate, and the angle range was recorded between 10° and 90° at an increment of 0.02° with locked scan type. The morphology as well as the elemental analysis for the surface of the corroded samples were investigated by the SEM and EDX; all images and spectra were obtained at 15 kV using SEM/EDX instruments purchased from JEOL (Tokyo, Japan).

3. Results and Discussion

3.1. XRD Patterns

XRD patterns collected for Ti-6%Al alloy (upper) and Ti-6%Al-4%V (bottom) are depicted in Figure 1. It is evident that the diffraction peaks that are corresponding to the Ti-6%Al alloy are Ti (see the powder diffraction standard for Ti, JCPDS No. 01-079-6208) and Al (see the powder diffraction standard for Al, JCPDS No. 01-074-5282). The Ti-6%Al-4%V alloy has also recorded the same aforementioned peaks in addition to the peak that is corresponding to vanadium or vanadium oxide (see the powder diffraction standard for V, JCPDS No. 01-086-2248). The XRD patterns confirmed the presence of all alloying elements; i.e., Ti, Al, and V, in the nanocomposites and at the exact compositions. Moreover, the XRD analysis has indicated that there were no contamination peaks observed as the result of the good preparation and mixing processes for the powders.

3.2. CPP Measurements

The CPP curves obtained for (1) Ti-6%Al and (2) Ti-6%Al-4%V after being immersed in the 3.5% NaCl solution for 1 h, respectively, are depicted in Figure 2. The CPP curves were also obtained after the alloy immersion in the same solution for 24 h and 48 h as seen from Figure 3 and Figure 4, respectively. The values of the cathodic and Tafel slopes, βc, βa, corrosion current and potential, j_Corr, E_Corr, corrosion rate, R_Corr, and polarization resistance, RP, all these values were manually collected from Figure 1, Figure 2 and Figure 3, and are seen in

Table 1. Polarization data for the Ti alloys after immersion in 3.5% NaCl solution for various periods of time.

Alloy/Time	Parameter
	βc/mV.dec−1	ECorr/mV	βa/mV.dec−1	jCorr/µA.cm−2	Rp/Ω.cm2	RCorr/mpy
Ti-6%Al/1 h	105	−330	130	4.30	587.3	0.3743
Ti-6%Al-4%V/1 h	90	−380	82	0.22	8480	0.0192
Ti-6%Al/24 h	110	−280	125	1.54	1652	0.1341
Ti-6%Al-4%V/24 h	105	−340	110	0.17	13,739	0.0148
Ti-6%Al/48 h	115	−310	135	0.56	4821	0.0487
Ti-6%Al-4%V/48 h	115	−400	125	0.15	17,361	0.0131

. It is worth mentioning that the βc, j_Corr, E_Corr, and βa value were calculated as have been reported in the previous research [37,40]. Moreover, the values of R_Corr and R_P were calculated using the following two equations [38,39]:

$$R_P=\frac{1}{j_{Corr}} \left(\frac{{\beta }_c.{\beta }_a}{2.3\left({\beta }_c+{\beta }_a\right)}\right),$$

(1)

$$R_{Corr}=j_{Corr}\left(\frac{k.E_W}{d.A}\right).$$

(2)

Here, k is a constant used to define the unit for R_Corr, E_W is the equivalent weight for the alloy(s), d represents the density of the alloy(s), and A is the surface area of the alloy(s) [38,39].

It is clear that the cathodic branch of the polarization curves shows a decrease in the currents with potential, where the cathodic reaction has reported to be the oxygen reduction reaction that can be represented as follows [43]:

$$2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2+4{\mathrm{e}}^{-}=4{\mathrm{OH}}^{-},$$

(3)

$$\frac{1}{2}\mathrm{O}+{\mathrm{H}}_2\mathrm{O}+2^{-}=2{\mathrm{OH}}^{-}.$$

(4)

The cathodic reaction may be undertaken by the reduction of oxygen, which will be adsorbed on the alloy’s surface as per the following reaction [5,7]:

$${\mathrm{OH}}_{\mathrm{ads}}+{\mathrm{e}}^{-}={\mathrm{OH}}^{-}.$$

(5)

The decrease of currents continued with scanning the potential in the forward direction until it reaches the value of E_Corr and j_Corr after which the anodic reaction starts. The anodic reaction for Ti-Al alloy has been reported to [44,45] take place via the dissolution of Al:

Al = Al³⁺ + 3e⁻.

(6)

The occurrence of this dissolution reaction increases the anodic currents, while the steady slowdown of the increase of current results from the adsorption of hydroxide ions on the surface to form aluminum hydroxide, Al(OH)_3ads as follows [46,47]:

$${\mathrm{Al}}_{\left(\mathrm{S}\right)}+3{\mathrm{OH}}^{-}=\mathrm{Al}{(\mathrm{OH})}_{3,\mathrm{ads}}+3{\mathrm{e}}^{-}.$$

(7)

The formed Al(OH)₃ is unstable and is transformed to hydrated oxide (Al₂O₃·3H₂O) [14]:

$$2\mathrm{Al}{(\mathrm{OH})}_{3,\mathrm{ads}}={\mathrm{Al}}_2{\mathrm{O}}_3.3{\mathrm{H}}_2\mathrm{O}.$$

(8)

Figure 2 reveals that the titanium alloy with only Al and Ti-6%Al shows higher absolute cathodic and anodic currents. Adding 4%V is seen to highly reduce the obtained currents and confirm that the presence of V decreases the reactions that take place at the cathode and anode and thus increases the alloys’ corrosion resistance. This was confirmed by the data listed in

Table 2. Impedance parameters for the tested alloys.

Alloy/Time	Impedance Data
	RS/Ω cm2	Q		RP1/Ω cm2	Cdl/F cm−2	RP2/Ω cm2
		YQ/S*s^n	n
Ti-6%Al/1 h	15.25	0.002573	0.42	440	0.00322	545
Ti-6%Al-4%V/1 h	19.91	0.000112	0.73	609	0.00018	5497
Ti-6%Al/24 h	17.82	0.002394	0.43	461	0.00569	602
Ti-6%Al-4%V/24 h	21.07	0.000678	0.78	981	0.00019	6185
Ti-6%Al/48 h	20.61	0.002346	0.47	537	0.00616	743
Ti-6%Al-4%V/48 h	24.58	0.000126	0.77	4203	0.00012	8035

, where the values of j_Corr and R_Corr were much lower for Ti-6%Al-4%V alloy as compared to their values for Ti-6%Al alloy. Table 2 also shows that the presence of V increases the value of R_P, which confirm the positive effect for V on decreasing the corrosion of the alloy in the 3.5% NaCl solution. In addition to the formation of Al₂O₃, titanium dioxide (TiO₂) may form on the surface of alloy because Ti alloys tend to form a spontaneous passive film of TiO₂ layer when its surface is exposed to air or being immersed in solution that contains water [10,48,49]. Accordingly, the surface of Ti gets oxidized first to form its cations (Ti²⁺) or reacts with the hydroxide ions formed in the cathodic reaction or may oxidize as per the following reactions [10,49]:

Ti = Ti²⁺ + 2e⁻,

(9)

2Ti_(S) + 4OH⁻ = 2Ti(OH)₂ + 4e⁻,

(10)

2Ti_(S) + 2O²⁻ = 2TiO_2(S) + 4e⁻.

(11)

Moreover, the presence of V increases the surface protection up to its additions due to the formation of V₂O₅ on the surface. This may lead to the increase of pitting corrosion, where the backward direction of the CPP curve recorded for Ti-6%Al-4%V alloy depicted the presence of a bigger hysteresis loop than the obtained one for Ti-6%Al. This may have resulted from the presence of both Ti and V together with Al leading to the increase of Al dissolution from the surface (reaction 6), which in turn leads to the increase of the pitting attack. The propagation of the pits after its initiation has been reported [46,50,51,52,53] to be attributed to the following reactions [43]:

Al₃⁺ + 3Cl⁻ = AlCl₃,

(12)

AlCl₃ + Cl⁻ = AlCl₄⁻.

(13)

AlCl₃ was formed due to the reaction between Al³⁺ and the chloride ions and would react with Cl⁻ to produce AlCl₄⁻ complex [47]. Another opinion stated that, instead of a direct reaction, the dissolution of the oxide film via the chemisorption of the Cl⁻ onto this film produces an oxychloride complex, Al(OH)₂Cl₂⁻, which causes the pitting [54,55,56];

2Al³⁺ + 2Cl⁻ + 2OH- = Al(OH)₂Cl₂⁻.

(14)

The CPP curves obtained after 24 h and 48 h (Figure 3 and Figure 4) decreased the cathodic currents, anodic currents, j_Corr and R_Corr and increased R_P, and this effect increases in the presence of V and the prolonging of time. Table 1 confirmed this finding as the values of j_Corr decreased from 4.3 µA/cm² for Ti-6%Al to be only 0.22 µA/cm² for Ti-6%Al-4%V. These values greatly decreased for both alloys with increasing time as listed in Table 1. On the other hand, the intensity of pitting corrosion was quite opposite for the long periods of immersed alloys, where, the increase of time increased the possibility of occurrence of pitting corrosion for Ti-6%Al alloy as indicated by the increase of the area of the obtained hysteresis loop with time, unlike the pitting corrosion, which, for Ti-6%Al-4%V, was found to decrease with time via decreasing the area of the hysteresis loop seen after 24 h and 48 h. The CPP results thus reveal that the presence of 4% V within the Ti-6%Al alloy highly decreases its corrosion, and this effect increases with increasing the immersion time to 24 h and much further to 48 h.

3.3. EIS Measurements

The Nyquist plots measurements for (1) Ti-6%Al alloy and (2) Ti-6%Al-4%V alloy immersed in 3.5% NaCl solution for 1 h are represented by Figure 5. Similar plots were measured for the same alloys in NaCl solution after 24 h and 48 h as seen by Figure 6 and Figure 7. These measurements were best fitted to a circuit model that is displayed in Figure 8, and the values of its parameters are recorded in Table 2. Here, R_S is the resistance of the test solution, C_dl is defined as the double layer capacitance, R_P1 is the polarization resistance, Q (YQ, CPEs) is considered as the constant phase elements, and R_P2 is the second polarization resistance [37].

The obtained spectra of Figure 5 show one semicircle, whether V is present or not. The presence of V is seen to greatly increase the corrosion resistance as indicated by the wide diameter of the semicircle that belongs to Ti-6%Al-4%V alloy. Another indication on the high corrosion resistance for the V containing alloy is values of the impedance parameters listed in Table 2, where the presence of V increased R_S, R_P1, and R_P2 values. Furthermore, the n value that accompany Q is circa 0.5 and can be considered as a Warburg impedance (W) in the case of Ti-6%Al alloy only. On the other side, in the case of a Ti-6%Al-4%V alloy, the value of n is > 0.75 and, therefore, its Q can be considered as a double layer capacitor with some pores. The presence of C_dl confirms also that the existence of V increases the resistance versus corrosion. Table 2 shows the decrease of Y_Q and C_dl values the presence of V, which further confirms the useful role of V on the protection of corrosion for the fabricated Ti-6%Al alloy.

As previously reported [57], the value of n varies between 0 and 1. If n = 1, then the behavior is related to an ideal capacitor, while if n value is closer to 1 and higher than 0.5, the behavior is a capacitor with some pores and is related to a non-uniform current caused by the inhomogeneities of the films or surface roughness distribution. If the value of n is around 0.5 means a Warburg impedance (W) and if n value is closer to 0, the system can be considered as an inductance.

As exhibited in Figure 6, the increase of immersion time to 24 h is seen to increase the width of the obtained semicircle of the Nyquist plots for (1) Ti-6%Al and (2) Ti-6%Al-4%V alloys. This effect was further increased to 48 h before measurement as depicted in Figure 7. The increase of immersion time thus increases the corrosion resistance of the alloys, which is certainly due to the development of thicker oxide films or corrosion product layer with time. The formed films or layers on the surface protect it from being attacked in the NaCl solution. This is supported by the data seen in Table 2, where all resistances are shown to increase and the values of Y_Q and C_dl decrease with the prolonging of the time of immersion as it is also increased due to the existence of V. The EIS obtained data thus confirm the polarization ones that the presence of 4% V highly enhances the resistance of the Ti-6%Al all against corrosion, and this effect greatly increased with prolonging the time of exposure from 1 h to 24 h and further to 48 h before collecting the measurements.

3.4. CCT Measurements

In order to confirm the effect of V addition on both the uniform corrosion and pitting attack at a constant anodic value of potential, CCT experiments were performed after various exposure times in the chloride test solution. The CCT plots seen in Figure 9 were recorded for (1) Ti-6%Al alloy and (2) Ti-6%Al-4%V alloy at 300 mV (Ag/AgCl) after immersion in 3.5% NaCl solution for 1 h. The obtained currents recorded an abrupt shift in the first few moments due to the dissolution of surface layer possibly forming as a result of immersing the alloys for 1 h before applying the positive potential. The current then slightly decreases with time because of the stabilization of the surface with an oxide film. For Ti-6%Al alloy, the current recorded high absolute values, while Ti-6%Al-V% alloy recorded very low currents. This indicates that the presence of 4%V highly increases the corrosion resistance of the titanium alloy. The current vs. time behavior also indicated that there is no pitting corrosion noticed for the surface of the alloys at the condition of 300 mV applied potential and 1 h immersion time.

Expanding the period of immersion time to 24 h (Figure 10) decreased the absolute currents for Ti-6%Al alloy and Ti-6%Al-4%V alloy meaning that the surface of the alloys developed an oxide film. This film gets thickened with time and leads to minimizing the attack on the surface of the alloys and reflects on the decrease of the obtained currents. This was further confirmed by prolonging the exposure period of time to 48 h as depicted in Figure 11, where the obtained currents were the minimum for both tested alloys. The most pronounced decreases in currents were recorded for a Ti-6%Al alloy, where it decreased from about 135 µA/cm² when it was exposed for 1 h to only 20 µA/cm² after 48 h exposure in the chloride solutions, while the decrease of currents for Ti-6%Al-4%V alloy was from circa 12 µA/cm² after 1 h immersion to about 4 µA/cm² after 48 h exposure in the chloride solutions before measurement. Therefore, the obtained currents decreased with time in the following order; 48 h < 24 h < 1 h as well as with the alloys as following; Ti-6%Al-4%V alloy < Ti-6%Al alloy. The chronoamperometric current–time measurements at +300 mV agree with the obtained results from CPP and EIS that the presence of 4% V greatly enhances the resistance towards corrosion of the titanium–aluminum alloy in the sodium chloride solution, and this effect highly enhanced when the exposure periods of time increases.

3.5. SEM and EDX Investigations

The SEM images together with EDX investigations were collected after performing the current-time experiments shown in Figure 12. Here, the alloys were exposed for 48 h in the 3.5% NaCl solutions before applying a constant value of potential at 300 mV for 30 min. Figure 12 shows (a) SEM and (b) EDX analysis for the surface of sintered Ti-6%Al alloy before its immersion; (b) SEM and (d) EDX analysis for the surface of the corroded Ti-6%Al alloy that was immersed in 3.5% NaCl solution for 48 h before stepping the potential at 300 mV for 30 min. It is seen that the SEM image for the sintered sample is smooth and has no signs on the occurrence of corrosion because it was not exposed to the test solution. On the other hand, the SEM image for the immersed sample (Figure 12c) has irregular corrosion products on the surface of the alloy, where there is an area that has a thick corrosion product layer and another area has some deposited sodium chloride salt. There are also some pits that appeared on the surface particularly, in the area that has no thick corrosion products. This confirms that the polarization measurements, where the hysteresis loop that appeared on the curve 1 of Figure 4 and the little increase of the current with time in some areas on curve 1 of Figure 11, revealed the occurrence of pitting corrosion. The weight percentages (wt.%) for the elements detected by EDX analysis depicted in Figure 12b were mainly the elements composed of the Ti-6Al alloy, while the wt.% of the corroded sample (Figure 12d) were 46.34% Ti, 30.95% O, 0.13% Al, 11.99% Na, and 10.59% Cl. The presence of this high % of oxygen indicates that the surface of covered with an oxide layer. This was confirmed by the lower % of Ti and Al than its initial % in the alloy. Oxides such as Al₂O₃ and TiO₂ may thus form on the surface of the Ti-6%Al alloy. The white corrosion product seen on the SEM image is most probably a deposited NaCl salt as the wt.% of both Na and Cl are nearly the same.

Figure 13 presents (a) the SEM and (b) the EDX analyses for the surface of sintered Ti-6%Al-4%V alloy before its immersion; (b) SEM and (d) EDX analysis for the surface of the corroded Ti-6%Al-4%V alloy that was immersed in 3.5% NaCl solution for 48 h before stepping the potential at 300 mV for 30 min. It is seen from the SEM images, whether it was immersed (Figure 13a) or not immersed in the test solution (Figure 13c), that the surface of the alloy is not attacked or pitted and seems to be homogeneous. The only difference between the two images is that the immersed sample has formed corrosion products due to the presence of the NaCl solution. The EDX profile analysis was then performed to ensure the composition of the alloy (Figure 13b) and whether corrosion product and/or oxide layers are formed on the surface in case of the immersed alloy (Figure 13d). The wt.% for the pure surface that has no corrosion products and that was not immersed in the chloride solution were almost the same as the main composition of the alloy. On the other hand, the wt.% detected for the elements of the corroded alloy using an EDX profile spectrum that is depicted in Figure 13d were as follows: 48.08% Ti, 30.15% O, 12.54% Al, 8.15% V, 0.62% Na, and 0.46% Cl. Here, the Ti% is lower, while the Al% is higher than expected. This may indicate the enrichment of Al on the surface as a result of its dissolution and then the formation of Al₂O₃ (reaction 8). The presence of almost double % the V than its actual % in the alloy may also indicate on the formation of V₂O₅ layer on the surface of the alloy. The formation of all these oxides and the disappearance of pits formation on the surface reflects on the higher corrosion resistance for Ti-6%Al-4%V alloy compared to Ti-6%Al alloy. The disappearance of the white corrosion product layer we have seen in the SEM image of Figure 12 is because the detected % for both Na and Cl were very low. The SEM/EDX investigations thus confirm that the presence of 4% V decreases the severity of corrosion in 3.5% NaCl and that effect is more pronounced after long immersion periods of time.

4. Conclusions

In this work, two titanium base alloys, namely Ti-6%Al alloy and Ti-6%Al-4%V alloy, were manufactured from their powders using the mechanical alloying technique. The XRD method confirmed the homogeneous distribution and the composition of the fabricated alloys. The corrosion in 3.5% NaCl solution of these alloys after 1 h, 24 h, and 48 h exposure was carried out using CPP, EIS, and CCT at 300 mV experiments. The corroded surfaces of the alloys were investigated using SEM micrographs and EDX profile analysis. All electrochemical (CPP, EIS, and CCT) measurements revealed that the presence of 4% V greatly decreased the corrosion of Ti-6%Al alloy via minimizing the values of corrosion current and the rate of this corrosion as well as increasing the values of polarization resistance. This was found to highly increase with prolonging the immersion time from 1 h to 24 h and the maximum resistance against corrosion for the Ti-6%Al alloy and Ti-6%Al-4%V alloy was obtained after their immersion in the 3.5% NaCl solution for 48 h. Moreover, the pitting corrosion was found to decrease with time for the Ti-6%Al-4%V alloy and increase for the Ti-6%Al alloy as revealed by the data of CPP and CCT. The results of SEM and EDX investigations indicated that the corrosion resistance of Ti-6%Al-4%V alloy was higher than the corrosion resistance of Ti-6%Al alloy due to the formation of a mixture of Al₂O₃, TiO₂, and V₂O₅ on the surface of the alloy.